You have a solution of KNO3 containing 28 g KNO3 in 100 g H2O at 30 degree C. Is the solution saturated or unsaturated? How many phases will be present in the solution? If saturated how much salute remains undissolved? (Help)

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anor277 Share
Apr 22, 2018

We have no data...

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Nitrates TEND to be soluble species...

And here we gots a concentration of ....

$\frac{\frac{28 \cdot g}{101.10 \cdot g \cdot m o {l}^{-} 1}}{100 \cdot m L \times {10}^{-} 3 \cdot L \cdot m {L}^{-} 1} = 2.77 \cdot m o l \cdot {L}^{-} 1$.

This site reports prodigious solubility....i.e. $360 \cdot g \cdot {L}^{-} 1$ at $20$ ""^@C...and it would be higher at $30$ ""^@C. And so, on this basis this solution is $\text{UNSATURATED}$ with respect to potassium nitrate: i.e. the solution contains an amount of solute LESS than that amount which would be in equilibrium with undissolved solute.

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